Answer
$N_{2}$ is $0.78\times 1.12 atm = 0.8736 atm$
$O_{2}$ is $0.22\times 1.12 atm =0.2464 atm $
Work Step by Step
Using Dalton's Law of Partial Pressure, we can find the pressure an individual gas exerts in a mixture of gases.
$Partial Pressure = Mole Fraction of Gas\times Total Pressure$
Since we are told that there is $22$ % of $O_{2}$ and $78$ % of $N_{2}$ , we can determine the mole fraction of each gas simply by converting the percent of $O_{2}$ and percent of $N_{2}$ gas into a number by dividing by 100 to get $0.22$ for $O_{2}$ and $0.78$ for $N_{2}$
Therefore, the partial pressure of $O_{2}$ is $0.22\times 1.12 atm =0.2464 atm $ and the partial pressure of $N_{2}$ is $0.78\times 1.12 atm = 0.8736 atm$
